Lithium nitride: Difference between revisions
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==Overview== | ==Overview== | ||
'''Lithium nitride''' is a [ | '''Lithium nitride''' is a [[Chemical compound|compound]] of [[lithium]] and [[nitrogen]] with the [[formula]] Li<sub>3</sub>N. It is the only stable [[alkali metal]] nitride. The solid is a red or purple color, has a high melting point and is ionic. It has an unusual crystal structure which consists of two different types of layer, one sheet, composition Li<sub>2</sub>N, containing 6 coordinate lithium ions and the other consisting only of lithium ions. Solid lithium nitride is a [[fast ion conductor]] and has the highest conductivity of any inorganic lithium salt. It has been studied extensively as a solid electrolyte and an anode material for use in batteries.<ref> US patent 4888258 (1989)</ref>. It can be formed by direct reaction of the elements, either by burning lithium metal in pure nitrogen gas or by reacting nitrogen gas with lithium dissolved in liquid [[sodium]] metal<ref> Barker M.G., Blake A.J, Edwards P.P., Gregory D.H., Hamor T. A., Siddons D. J., Smith S. E. Chem. Commun., 1999, 1187–1188</ref>. The second method gives a purer product. Lithium nitride reacts violently with [[water]] to produce [[ammonia]]: | ||
All ionic nitrides display this pattern, due to the N<sup>3<nowiki>−</nowiki></sup> ion being an extremely strong Bronsted [ | Li<sub>3</sub>N (s) + 3 H<sub>2</sub>O (l) → 3 LiOH (aq) + NH<sub>3</sub> (g) | ||
All ionic nitrides display this pattern, due to the N<sup>3<nowiki>−</nowiki></sup> ion being an extremely strong Bronsted [[Base (chemistry)|base]]. It easily qualifies as a [[superbase]]. It is, in fact, a stronger base than the [[hydride]] ion, so deprotonates hydrogen itself: | |||
Li<sub>3</sub>N (s) + 2 H<sub>2</sub> (g) → LiNH<sub>2</sub> (s) + 2 LiH (s). | Li<sub>3</sub>N (s) + 2 H<sub>2</sub> (g) → LiNH<sub>2</sub> (s) + 2 LiH (s). | ||
Lithium nitride is being investigated as a potential [ | Lithium nitride is being investigated as a potential [[hydrogen storage|storage medium]] for [[hydrogen]] gas, as the reaction is reversible at 270<sup>o</sup>C. Up to 11.5% by weight absorption of hydrogen has been achieved<ref>Ping Chen, Zhitao Xiong, Jizhong Luo, Jianyi Lin and Kuang Lee Tan. Nature, November 21, 2002.</ref>. | ||
==References== | ==References== | ||
* [http:// | * [http://www.webelements.com/ WebElements] | ||
*{{Greenwood&Earnshaw}} | *{{Greenwood&Earnshaw}} | ||
<references /> | <references /> | ||
[ | [[Category:Nitrides]] | ||
[[Category:Lithium compounds]] | |||
{{inorganic-compound-stub}} | {{inorganic-compound-stub}} | ||
[ | [[ar:نتريد ليثيوم]] | ||
[ | [[de:Lithiumnitrid]] | ||
[[ja:窒化リチウム]] | |||
[[vi:Nitrua liti]] | |||
{{WH}} | {{WH}} | ||
{{WS}} | {{WS}} | ||
Revision as of 23:36, 6 January 2011
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Overview
Lithium nitride is a compound of lithium and nitrogen with the formula Li3N. It is the only stable alkali metal nitride. The solid is a red or purple color, has a high melting point and is ionic. It has an unusual crystal structure which consists of two different types of layer, one sheet, composition Li2N, containing 6 coordinate lithium ions and the other consisting only of lithium ions. Solid lithium nitride is a fast ion conductor and has the highest conductivity of any inorganic lithium salt. It has been studied extensively as a solid electrolyte and an anode material for use in batteries.[1]. It can be formed by direct reaction of the elements, either by burning lithium metal in pure nitrogen gas or by reacting nitrogen gas with lithium dissolved in liquid sodium metal[2]. The second method gives a purer product. Lithium nitride reacts violently with water to produce ammonia:
Li3N (s) + 3 H2O (l) → 3 LiOH (aq) + NH3 (g)
All ionic nitrides display this pattern, due to the N3− ion being an extremely strong Bronsted base. It easily qualifies as a superbase. It is, in fact, a stronger base than the hydride ion, so deprotonates hydrogen itself:
Li3N (s) + 2 H2 (g) → LiNH2 (s) + 2 LiH (s).
Lithium nitride is being investigated as a potential storage medium for hydrogen gas, as the reaction is reversible at 270oC. Up to 11.5% by weight absorption of hydrogen has been achieved[3].